Coper metal can reduce `Fe^(2+)` in acidic medium.

Explanation

To determine whether copper metal can reduce \( \text{Fe}^{2+} \) in acidic medium, we need to analyze the electrochemical properties of copper and iron.

### Step-by-Step Solution:

1. **Understand the Reduction Reaction**:
- A reduction reaction involves the gain of electrons. In this case, we are looking at whether copper can reduce \( \text{Fe}^{2+} \) to iron metal (Fe).
- The half-reaction for the reduction of \( \text{Fe}^{2+} \) is:
\[ \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \]

2. **Identify the Oxidation States**:
- In the reaction, \( \text{Fe}^{2+} \) is in the +2 oxidation state, and iron (Fe) is in the 0 oxidation state when it is in its elemental form.

3. **Refer to the Electrochemical Series**:
- The electrochemical series ranks metals based on their standard electrode potentials. The more positive the potential, the more likely the species is to be reduced.
- Copper (Cu) has a standard reduction potential of \( +0.34 \, \text{V} \) for the half-reaction:
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \]
- Iron (Fe) has a standard reduction potential of \( +0.77 \, \text{V} \) for the half-reaction:
\[ \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \]

4. **Compare the Potentials**:
- Since the standard reduction potential for \( \text{Fe}^{2+} \) is higher than that for \( \text{Cu}^{2+} \), this indicates that \( \text{Fe}^{2+} \) is a stronger oxidizing agent than \( \text{Cu}^{2+} \).
- Therefore, copper cannot reduce \( \text{Fe}^{2+} \) because it does not have a sufficient driving force (i.e., it cannot provide the necessary electrons).

5. **Conclusion**:
- Since copper cannot reduce \( \text{Fe}^{2+} \) to iron, the statement is false. Copper is less reactive than iron and cannot displace iron from its salts.

### Final Answer:
Copper metal cannot reduce \( \text{Fe}^{2+} \) in acidic medium. This statement is false.